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Molecular Compounds: Formulas & Naming

Molecular Compounds: Formulas & Naming. Ch 6.3b - Covalent Bonds. What type of bond?. Covalent Electrons are shared between atoms Forms between non-metals Covalent Bonds  Molecular Compounds Which elements are non-metals?. Describing Molecular Compounds.

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Molecular Compounds: Formulas & Naming

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  1. Molecular Compounds: Formulas & Naming Ch 6.3b - Covalent Bonds

  2. What type of bond? • Covalent • Electrons are shared between atoms • Forms between non-metals • Covalent Bonds  Molecular Compounds • Which elements are non-metals?

  3. Describing Molecular Compounds • What information do the name and formula of a molecular compound provide? • Ionic Bonds (Ionic Compounds) - • The name distinguishes the compound from other ionic compounds containing the same elements. • The formulaof an ionic compound describes the ratio of the ions in the compound.

  4. Describing Molecular Compounds • Covalent Bonds (Molecular Compounds) • The name and formula of a molecular compound describe the type and number of atoms in a molecule of the compound.

  5. Naming Molecular Compounds Naming Order: Step 1: Element that is farthest to the left side of the periodic table is typically named 1st. (left to right) The most metallic element appears first in the name. These elements are farther to the left in the periodic table. If both elements are in the same group, the more metallic element is closer to the bottom of the group. Formulas are written same way Example: Sulfur is named before chlorine  SCl2

  6. Naming Molecular Compounds • Exception: Oxygen & Halogens • Oxygen comes 2nd when combined with lower-electronegativity halogens (Group 17) • Example: ClO2 (electronegativity: Cl = 3.0; O = 3.5) • Step 2: Second element name is changed to end in “ide” (like the anion in an ionic compound) • Examples: • Chlorine becomes chloride • Oxygen becomes oxide

  7. Naming Molecular Compounds mono - one di - two tri - three tetra - four penta - five hexa - six hepta - seven octa - eight nona - nine deca - ten • There may be more than one molecular compound that can exist with the same two elements. • Greek prefixes are used to name molecular compounds. • Step 3: Add prefixes to elements names to specify the number of atoms of each element in the compound.

  8. Prefixes: mono - one di - two tri - three tetra - four penta - five Example: Both Compounds contain Nitrogen and Oxygen N2O  Dinitrogen monoxide N4O5 Tetranitrogen pentoxide Naming Molecular Compounds

  9. Naming Molecular Compounds • Exception to Step 3– No prefix is used if there is only one atom of the 1st element in the compound. • CO  Carbon monoxide • CO2 Carbon dioxide • SO10 Sulfur decaoxide

  10. N2Cl5 Dinitrogen pentachloride N2O5 Dinitrogen pentoxide P5Cl6 Pentaphosphorous hexachloride SO10 Sulfur decaoxide Naming Molecular CompoundsMore Examples:

  11. Writing Molecular Formulas • Step 1: Write the symbols for the elements in the order the elements appear in the name. • Step 2: Write the numerical value of the prefixes as subscripts for the corresponding element in the formulas. • The prefixes indicate the number of atoms of each element in the molecule. • If there is no prefix for an element in the name, there is only one atom of that element in the molecule.

  12. Writing Molecular Formulas • Examples: • Diphosphorus Pentoxide  P2O5 • Silcon Dioxide  SiO2 • Carbon Tetrachloride  CCl4 • Trineptunium Octoxide  Np3O8

  13. You Try • Give the formula for: • Oxygen Difluoride  • Phosphorus Tribromide  • Trisilicon Tetranitride  • Give the Name for: • NO2  • N2O3  • SO3 

  14. You Try - Answers • Give the formula for: • Oxygen Difluoride  OF2 • Phosphorus Tribromide  PBr3 • Trisilicon Tetranitride  Si3N4 • Give the Name for: • NO2  Nitrogen Dioxide • N2O3  Dinitrogen Trioxide • SO3  Sulfur Trioxide

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